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APS104H1 Study Guide - Quiz Guide: Van Der Waals Equation, Ideal Gas Law, Isothermal Process

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tealdolphin707
16 Oct 2011
School
UTSG
Department
Chemical Engineering and Applied Chemistry
Course
APS104H1
Professor
Edgar Acosta

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Document Summary

Closed system: exchange of energy but not mass. Isolated system: no exchange of anything at all. Adiabatic system: no not allow heat exchange between the system and surroundings. Isothermal system: allows exchange of heat b/w system and surroundings. Zeroth law of thermodynamics: states that if system a is in equilibrium with b and b is in equilibrium with c then a is also in equilibrium with c. You have the ideal gas law where you have pv=nrt where p is pressure, v is volume, n is number of moles, r is the constant, and t is the temperature in kelvin. Number of moles is also given by the equation n= where m is the mass and m is the molar mass. Also there is the concept of partial pressure where you have: You have the van der waals equation as well which works for only mixtures: Another equation which works with the ideal gas law is:

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Related Questions

Define the terms system and surroundings. What does it mean to say that a system and its surroundings are in thermal equilibrium?

 

1.) For a reaction system that is at equilibrium, which of the following must always be true?
a. q = 0 b. ?S = 0 c. ?G = 0 d. ?H = 0


2.) A certain reaction is found to be reactant favored. Which of the following is a correct description of the
reaction?
a. ?G° > 0, K > 1 b. ?G° > 0, K < 1 c. ?G° < 0, K > 1 d. ?G° < 0, K < 1


3.) What does the third law of thermodynamics state?
a. It states that a substance that is perfectly crystalline at 0 K has an entropy of zero.
b. It states that if two systems are each in thermal equilibrium with a third, they are also in thermal
equilibrium with each other.
c. It states that any quantity which has a continuous differentiable symmetry in the action has an
associated conservation law.
d. It states that the increase in internal energy of a closed system is equal to the difference between
the heat supplied to the system and the work done by the system.

If you add boiling water to a cup at room temperature, what would you expect the final equilibrium temperature of the unit to be? You will need to include the surroundings as a pan of the system. Consider the zeroth law of thermodynamics.